1. Why do Titration Curves Look Like THAT ???? 1/4/20161

2. Calculate the pH when the following quantities of 0.100 M NaOH solution have been added to 50.0 mL of 0.100 M HCl solution: A. 30.0 mL B, 49.0 mL C. 49.5 mL D. 50.0 mL E. 50.5 mL F. 60.0 mL 1/4/20162

3. Solution for 30.0 mL NaOH  Both Na + and Cl - are spectator ions.  Find how many moles H + and moles OH - present, then calculate how many mole of each ion remain after neutralization. BeforeChangeRemaining H+ 0.005-0.0030.002 OH- 0.003-0.0030 1/4/2016 3

4. Remaining H+ mole / new soln volume New pH now… 1/4/20164

5. Solution for 49.0 mL NaOH BeforeChangeRemaining H+ 0.005-0.00490.0001 OH- 0.0049-0.00490 1/4/2016 5

6. Remaining H+ mole / new soln volume New pH now… 1/4/20166

7. Solution for 49.5 mL NaOH BeforeChangeRemaining H+ 0.005-0.004950.00005 OH- 0.0049-0.004950 1/4/2016 7

8. Remaining H+ mole / new soln volume New pH now… 1/4/20168

9. Solution for 50.0 mL NaOH BeforeChangeRemaining H+ 0.005-0.0050 OH- 0.005-0.0050 1/4/2016 9

10. [H + ] = [OH - ] = 0 M Neutral pH = 7 New pH now… 1/4/201610

11. Solution for 50.5 mL NaOH BeforeChangeRemaining H+ 0.005-0.0050 OH- 0.00505-0.0050.00005 1/4/2016 11

12. Remaining OH- mole / new soln volume New pH now… 1/4/201612

13. Solution for 60.0 mL NaOH BeforeChangeRemaining H+ 0.005-0.0050 OH- 0.006-0.0050.001 1/4/2016 13

14. Remaining OH- mole / new soln volume New pH now… 1/4/201614

15. 1/4/201615 Titration curve for a strong acid by a strong base Any indicator that changes color along the steep portion of the titration curve is suitable for the titration. Methyl violet changes color too soon, and alizarin yellow R too late.

16. Subtle vocabulary point  Equivalence point: where equal moles of acid and base are present.  End Point: where an indicator chemical changes color. It may not be exactly at the equivalence point, but generally very close. 1/4/2016 16

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